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The isomerization of methylisonitrile to acetonitrile CH3NC(g) → CH3CN(g) is first order in CH3NC. The rate constant for the reaction is 9.45 × 10-5 s-1 at 478 K. The half-life of the reaction when the initial [CH3NC] is 0.030 M is ________ s

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Answer: The half-life of the reaction is 7333 seconds

Step-by-step explanation:

Expression for rate law for first order kinetics is given by:


t=(2.303)/(k)\log(a)/(a-x)

where,

k = rate constant

t = age of sample

a = let initial amount of the reactant

a - x = amount left after decay process

a) for completion of half life:

Half life is the amount of time taken by a radioactive material to decay to half of its original value.


t_{(1)/(2)}=(0.693)/(k)


t_{(1)/(2)}=(0.693)/(9.45* 10^(-5))=7333s

The half-life of the reaction is 7333 seconds

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